An equilibrium mixture of CO, O2, and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0020 M O2. At this temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). What is the equilibrium concentration of CO?

Given the equilibrium expression 0.0611 = x^2 / ((1370 - x)(1710 - x)), what is the value of x at equilibrium?

Given the equilibrium reaction 2CO(g) + O2(g) ⇌ 2CO2(g) with Kc = 2.8 × 10^2 at 298 K, and the partial pressures of CO and O2 are 5.168 × 10^-8 torr and 0.988 torr respectively, what is the partial pressure of CO2 in this mixture?

At a certain temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?

A solution initially contains [Ag+] of 3.2 × 10^-3 M and 0.125 M NH3. What is the concentration of Ag+ after the solution reaches equilibrium, given that the formation constant (Kf) of Ag(NH3)2+ is 1.7 × 10^7?

At a certain temperature, the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

What is the equilibrium constant expression for a reaction at equilibrium?

Calculate the equilibrium constant (K) for the reaction: 2 N2O (g) + 3 O2 (g) ⇌ 2 N2O4 (g), using the following information: 1) 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) K1 = 1.2 x 10^-35 2) N2O4 (g) ⇌ 2 NO2 (g) K2 = 4.6 x 10^-3 3) ½ N2 (g) + O2 (g) ⇌ NO2 (g) K3 = 4.1 x 10^-9

Given the equilibrium reaction: H₂C₂O₄ ⇌ 2H⁺ + C₂O₄²⁻, calculate the equilibrium concentration of C₂O₄²⁻ in a 0.20 M solution of oxalic acid, assuming the acid dissociates completely. The equilibrium constant, Kₐ, for the first dissociation is 5.5 x 10⁻².